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Standard Gibbs energy change and the equilibrium constant

This type of question, asked 5 times: 10 May 2023 S2, 11 Apr 2026 S2, 19 Apr 2026 S1, 19 Apr 2026 S2, 20 Apr 2026 S1. All 5 questions below, oldest first.

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  1. Question 1

    10 May 2023 S2

    85
    For the reaction CH4(g)+H2(g)→C2H6(g)\text{CH}_4(\text{g}) + \text{H}_2(\text{g}) \rightarrow \text{C}_2\text{H}_6(\text{g}), Kp=3.356×1017K_p = 3.356 \times 10^{17}, calculate ΔG∘\Delta G^\circ for the reaction at 298 K.

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  2. Question 2

    11 Apr 2026 S2

    6
    The equilibrium constant for a reaction is 100100. What will be the value of standard Gibbs energy change at 298298 K ? (R=8.314 J K−1mol−1)(R = 8.314\ \mathrm{J\,K^{-1}mol^{-1}})

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  3. Question 3

    19 Apr 2026 S1

    8
    Identify from following, the relation between standard free energy change in a reaction and equilibrium constant KcK_c.

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  4. Question 4

    19 Apr 2026 S2

    7
    Calculate standard Gibbs energy for any gaseous reaction if values of KpK_p and RR respectively are 3.5×10173.5 \times 10^{17} ; 8.314 JK−1mol−18.314\ \mathrm{JK^{-1}mol^{-1}}

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  5. Question 5

    20 Apr 2026 S1

    8
    Calculate ΔG∘\Delta G^\circ for reaction, CH4(g)+H2(g)→C2H6(g)\mathrm{CH_{4(g)} + H_{2(g)} \rightarrow C_2H_{6(g)}} (Kp=2×1017,R=8.314 JK−1mol−1)(K_p = 2 \times 10^{17}, R = 8.314\ \mathrm{JK^{-1}mol^{-1}})

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